What is the mass of silver that can be prepared from 2.10 g of copper metal? cu(s)+2agno3(aq)→cu(no3)2(aq)+2ag(s )

 The mass  of silver that can be prepared from 2.10 g of copper  metal are  7.128  grams  of Ag

 calculation

 Cu(s)  + 2AgNO3 (aq)  →  Cu(NO3)2  +2 Ag (s)

  find the moles of Cu

 = mass/ molar mass

= 2.10 g / 63.5 g/mol = 0.033  moles

Use the mole  ratio to determine  the  moles of Ag

The mole ratio of Cu : Ag is  1:2 therefore the moles of Ag = 0.033 x2=0.066 moles

mass of Ag =  moles x molar  mass

= 0.066 moles x  108   g/mol  = 7.128   grams of Ag

the answer is either b or c

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.